12: Acids, Bases, and Buffers
- Page ID
- 288497
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- 12.1: Arrhenius Definition of Acids and Bases
- Arrhenius acid: a compound that increases the concentration of hydrogen ion (H+) in aqueous solution; Arrhenius base: a compound that increases the concentration of hydroxide ion (OH−) in aqueous solution. the reaction of an acid and a base
- 12.2: Brønsted-Lowry Definition of Acids and Bases
- A Brønsted-Lowry acid is a proton donor, and a Brønsted-Lowry base is a proton acceptor. Brønsted-Lowry acid-base reactions are essentially proton transfer reactions.
- 12.3: Water - Both an Acid and a Base
- Water molecules can act as both an acid and a base, depending on the conditions.
- 12.4: The Strengths of Acids and Bases
- Acids and bases can be strong or weak depending on the extent of ionization in solution. Most chemical reactions reach equilibrium at which point there is no net change. The pH scale is used to succinctly communicate the acidity or basicity of a solution.
- 12.5: Buffers
- A buffer is a solution that resists sudden changes in pH.